Using bond-energy data,what is ΔH° for the following reaction?
CH₄(g) + 2F₂(g) → CF₄(g) + 2H₂(g)
Bond
Bond Energy (kJ/mol)
C-H
413
H-H
432
F-F
159
C-F
485

Question

Quizplus · Accepted Answer

The correct answer is A because the ΔH° for the reaction is -834 kJ. This can be calculated using the bond energies of the reactants and products:ΔH° = Σ(bond energies of reactants) - Σ(bond energies of products)ΔH° = [(4 × 413 kJ/mol) + (2 × 159 kJ/mol)] - [(4 × 485 kJ/mol) + (2 × 432 kJ/mol)]ΔH° = -834 kJ

Using Bond-Energy Data,what Is ΔH° for the Following Reaction